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A Level Chemistry (OCR) - Memorise > A1 Definitions > Flashcards

A1 Definitions Flashcards

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1
Q

Acid

A

A species that releases H+ ions in aqueous solution

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2
Q

Activation energy Ea

A

The minimum energy required to start a reaction by the breaking of bonds

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3
Q

Actual yield

A

The amount of product obtained from a reaction

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4
Q

Addition polymerisation

A

Formation of a very long molecular chain (addition polymer) by repeated addition reactions of many unsaturated alkene molecules called monomers

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5
Q

Addition reaction

A

A reaction in which a reactant is added to an unsaturated molecule to make one saturated molecule

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6
Q

Adsorption

A

The process that occurs when a gas or liquid or solute is held onto the surface of a solid

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7
Q

Alicyclic

A

Containing carbon atoms joined together in a ring that is not aromatic

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8
Q

Aliphatic

A

Containing carbon atoms joined together in unbranched (straight) or branched chains

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9
Q

Alkali

A

A type of base that dissolves in water to release hydroxide ions

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10
Q

Alkanes

A

The hydrocarbon homologous series with the general formula CnH2n+2

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11
Q

Alkenes

A

The hydrocarbon homologous series with one double carbon to carbon bond and the general formula CnH2n

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12
Q

Alkyl group

A

A side chain formed by removing a hydrogen atom from an alkane parent chain. Any alkyl group is often shown as ‘R’

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13
Q

Alkynes

A

The hydrocarbon homologous series with one triple carbon-to-carbon bond and the general formula CnH2n-2

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14
Q

Amount of substance n

A

The quantity whose unit of the mole. Chemists use amount of substance as a means of counting atoms.

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15
Q

Anhydrous

A

Containing no water molecules

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16
Q

Anion

A

A negatively charged ion with more electrons than protons

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17
Q

Aromatic

A

Containing one or more benzene rings

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18
Q

Atom economy

A

Sum of molar mass of desired products/ Sum of molar mass of all products, MULTIPY BY 100 FOR A PERCENTAGE

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19
Q

Atomic number Z

A

The number of protons in the nucleus of an atom

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20
Q

Atomic orbital

A

A region around the nucleus that can hold up to two electrons, with opposite spins

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21
Q

Average bond enthalpy

A

The average enthalpy change that takes place when breaking by homolytic fission one mole of a given type of bond in the molecules of a gaseous species

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22
Q

Avogadro constant NA

A

6.02x10^23 mol-1, the number of atoms per mole of carbon-12

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23
Q

Avogadro’s hypothesis

A

Equal volumes of gases at the same temperature and pressure contain the same number of molecules

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24
Q

Base

A

A compound that neutralises an acid to form a salt

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25
Q

Binary compound

A

A compound containing two elements only

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26
Q

Bond angle

A

The angle between two bonds in an atom

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27
Q

Bonded pair

A

A pair of electrons shared between two atoms to make a covalent bond

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28
Q

Carbocation

A

An ion that contains a positively charged carbon atom

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29
Q

Catalyst

A

A substance that increases the rate of a chemical reaction without being used up in the process. A catalyst provides an alternative route for the reaction with a lower activation energy

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30
Q

Cation

A

A positively charged ion with fewer electrons than protons

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31
Q

Chain reaction

A

A reaction in which the propagation steps release new radicals that continue the reaction

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32
Q

Cis-trans isomerism

A

A special type of E/Z isomerism in which there are two non-hydrogen groups and two hydrogen atoms around the C=C double bond

Cis - Z isomer (same side)
Trans - E isomer (different side)

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33
Q

Closed system

A

A system isolated from its surroundings

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34
Q

Collision theory

A

Two reacting particles must collide for a reaction to occur and must be in the correct orientation and have sufficient energy to overcome the activation energy of the reaction.

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35
Q

Coordinate bond

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only. Also called a dative covalent bond

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36
Q

Covalent bonding

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

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37
Q

Dative covalent bond

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only. Also called a coordinate bond

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38
Q

Dehydration

A

An elimination reaction in which water is removed from a saturated molecule to make an unsaturated molecule.

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39
Q

Delocalised electrons

A

Electrons that are shared between more than two atoms

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40
Q

Desorption

A

Release of an adsorbed substance from a surface

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41
Q

Dipole

A

A separation in electrical charge so that one atom of a polar covalent bond, or one end of a polar molecule, has a small positive charge 𝛿+ and the other has a small negative charge 𝛿-

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42
Q

Dipole-dipole force

A

An attractive force between permanent dipoles in neighbouring polar molecules.

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43
Q

Displacement reaction

A

A reaction in which a more reactive element displaces a less reactive element from an aqueous solution of its ions

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44
Q

Displayed formula

A

A formula that shows the relative positioning of all the atoms in a molecule and the bonds between them.

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45
Q

Disproportionation

A

A redox reaction in which the same element is both oxidised and reduced

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46
Q

Dynamic equilibrium

A

The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and concentrations do not change

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47
Q

E/Z isomerism

A

A type of stereoisomerism in which different groups attached to each carbon of a C=C double bond may be arranged differently in space because of the restricted rotation of the C=C bond

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48
Q

Electron configuration

A

A shorthand method for showing how electrons occupy sub-shells in an atom.

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49
Q

Electronegativity

A

A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond

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50
Q

Electrophile

A

An atom or group of atoms which is attracted to an electron-rich centre where it accepts a pair of electrons

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51
Q

Electrophilic addition

A

An addition reaction in which the first step is attack by an electrophile on a region of high electron density

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52
Q

Elimination reaction

A

The removal of a molecule from a saturated molecule to make an unsaturated molecule

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53
Q

Empirical formula

A

A formula that shows the simplest whole-number ratio of atoms of each element present in a compound

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54
Q

End point

A

The point in a titration where the indicator changes colour; the end point indicates when the reaction is just complete

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55
Q

Endothermic reaction

A

A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants resulting in heat being taken in from the surroundings (ΔH is positive)

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56
Q

Enthalpy

A

The heat content that is stored in a chemical system

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57
Q

Enthalpy change ΔH

A

Difference in enthalpy between reactants and products in a reaction

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58
Q

Enthalpy cycle

A

A diagram showing alternative routes between reactants and products which allows the indirect determination of an enthalpy change from other known enthalpy changes using Hess’ law.

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59
Q

Enthalpy profile diagram

A

A diagram for a reaction to compare the enthalpy of the reactants with the enthalpy of the products

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60
Q

Equilibrium constant Kc

A

A measure of the position of equilibrium; the magnitude of an equilibrium constant indicates whether there are more reactants or more products in an equilibrium system

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61
Q

Exothermic reaction

A

A reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants resulting in heat loss to the surroundings ΔH is negative

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62
Q

Fingerprint region

A

An area of an infrared spectrum below 1500cm^-1 that gives a characteristic pattern for different compounds

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63
Q

First ionisation energy

A

The energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions

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64
Q

Fractional distillation

A

The separation of components in a liquid mixture by their different boiling points into fractions with different compositions

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65
Q

Fragment ions

A

Ions formed from the breakdown of the molecular ion in a mass spectrometer

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66
Q

Fragmentation

A

The process in mass spectrometry that causes a positive ion to split into smaller pieces, one of which is a positive fragment ion.

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67
Q

Functional group

A

The part of the organic molecule responsible for its chemical reactions

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68
Q

General formula

A

The simplest algebraic formula of a member of a homologous series.

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69
Q

Giant covalent lattice

A

A three-dimensional structure of atoms, bonded together by strong covalent bonds

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70
Q

Giant ionic lattice

A

A three-dimensional structure of atoms, bonded together by strong covalent bonds

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71
Q

Giant ionic lattice

A

A three dimensional structure of atoms, bonded together by strong ionic bonds

72
Q

Giant metallic lattice

A

A three-dimensional structure of positive ions and delocalised electronsm bonded together by strong metallic bonds

73
Q

Group

A

A vertical column in the periodic table.

Elements in a group have similar chemical properties and their atoms have the same number of outer shell electrons

74
Q

Hess’ law

A

If a reaction can take place by more than one route and the initial and final conditions are thee same, the total enthalpy change is the same for each route

75
Q

Heterogeneous catalysis

A

A reaction in which the catalyst has a different physical state from the reactants; frequently reactants are gases whilst the catalyst is a solid

76
Q

Heterolytic fission

A

The breaking of a covalent bond forming a cation (+) and an anion (-)

77
Q

Homogeneous catalysis

A

A reaction in which the catalyst and reactants are in the same physical state, which is most frequently the aqueous or gaseous state

78
Q

Homologous series

A

A series of organic compounds with the same functional group but with each successive member differing by CH2

79
Q

Homolytic fission

A

The breaking of a covalent bond with one of the bonded electrons going to each atom, forming two radicals

80
Q

Hydrated

A

A crystalline compound containing water molecules

81
Q

Hydrocarbon

A

A compound containing carbon and hydrogen only

82
Q

Hydrogen bond

A

A strong dipole dipole attraction between an electron-deficient hydrogen atom of -NH, -OH, or HF on one molecule and a lone pair of electrons on a highly electronegative atom containing N, O or F on a different molecule

83
Q

Hydrolysis

A

A reaction with water that breaks a chemical compound into two compounds, the H and OH in a water molecule becomes incorporated into the two compounds

84
Q

Induced dipole-dipole interaction

A

Attractive forces between induced dipoles in different molecules, also known as LONDON FORCES

85
Q

Initiation

A

The first stage in a radical reaction in which radicals start when a covalent bond is broken by homolytic fission of a covalent bond

86
Q

Intermediate

A

A species formed during a reaction that reacts further and is not present in the final products

87
Q

Intermolecular forces

A

An attractive force between molecules. Intermolecular forces can be London Forces, Permanent Dipole-Dipole Interactions or Hydrogen Bonding

88
Q

Ion

A

A positively or negatively charged atom or a covalently bonded group of atoms (polyatomic ion), where the number of electrons is different from the number of protons.

89
Q

Ionic bonding

A

The electrostatic attraction between oppositely charged ions.

90
Q

Isotope

A

Atoms of the same element with different numbers of neutrons and different masses.

91
Q

Le Chatelier’s principle

A

When a system in dynamic equilibrium is subjected to an external change, the system readjusts itself to minimise the effect of the change and to restore equilibrium

92
Q

Limiting reagent

A

The reactant that is not in excess, which will be used up first and stop the reaction

93
Q

London forces

A

Attractive forces between induced dipoles in different molecules; also known as induced dipole-dipole interactions

94
Q

Lone pair

A

An outer shell pair of electrons that is not involved in chemical bonding

95
Q

Mass number A

A

The sum of the number of protons and neutrons in trhe nucleus; also known as a nucleon number

96
Q

Metallic bonding

A

The electrostatic attraction between positive metal ions and delocalised electrons

97
Q

Concentration

A

The amount of solute, in moles, dissolved in 1dm^3 of solution

98
Q

Molar gas volume Vm

A

The volume per mole of gas molecules at a stated temperature and pressure.

99
Q

Molar mass M

A

The mass per mole of a substance in units of g mol^-1

100
Q

Mole

A

The amount of any substance containing as many elementary particles as there are carbon atoms in exactly 12g of the carbon-12 isotope, ie. 8.02x^23 particles

101
Q

Molecular formula

A

A formula that shows the number and type of atoms of each element present in a molecule

102
Q

Molecular ion

A

The positive ion formed in mass spectrometry when a molecule loses an electron

103
Q

Molecule

A

The smallest part of a covalent compound that can exist while retaining its chemical identity, consisting of two or more atoms covalently bonded together

104
Q

Monomer

A

A small molecule that combines with many other monomers to form a polymer

105
Q

Neutralisation

A

The reaction between an acid and a base to produce a salt

106
Q

Nomenclature

A

A system of naming compounds

107
Q

Non-polar

A

With no charge separation across a bond or in a molecule

108
Q

Nucleon number

A

The number of protons and neutrons in an atom

109
Q

Nucleophile

A

An atom or group of atoms that is attracted to an electron-deficient carbon atom where it donates a pair of electrons to form a new covalent bond

110
Q

Nucleophilic substitution

A

A reaction in which a nucleophile is attracted to an electron-deficient carbon atom and replaces an atom or group of atoms on it

111
Q

Oxidation

A

Loss of electrons or an increase in oxidation number

112
Q

Oxidation number

A

A measure of the number of electrons that n atom uses to bond with atoms of another element. Oxidation numbers are derived from a set of rules

113
Q

Oxidation state

A

The oxidation number

114
Q

Oxidising agent

A

A reagent that oxidises (takes electrons from) another species

115
Q

π-bond

A

A bond formed by the sideways overlap of two p orbitals, containing two electrons and with the electron density concentrated above and below the line joining the nuclei of the bonding atoms

116
Q

Partial dissociation

A

The splitting of some of a species in solution into aqueous ions

117
Q

Pauling electronegativity value

A

A value assigned as a measure of the relative attraction of a bonded atom for the pair of electrons in a covalent bond

118
Q

Percentage yield

A

Actual yield divided by theoretical yield

Multiply by 100

119
Q

Periodicity

A

A repeating trend in properties of the elements across each period of the periodic table

120
Q

Periods

A

A horizontal row of elements in the periodic table. Elements show trend in properties across a period

121
Q

Permanent dipole

A

A small charge difference that does not change across a bond, with positive and negative partial changes on the bonded atoms: the result of the bonded atoms having different electronegativities

122
Q

Permanent dipole-dipole interactions

A

Attractive forces between the permanent dipoles in different molecules

123
Q

Polar molecule

A

A molecule with an overall dipole, having taken into account any dipoles across bonds and the shape of the molecule

124
Q

Polar covalent bond

A

A bond with a permanent dipole, having positive and negative partial charges on the bonded atoms

125
Q

Polyatomic ion

A

An ion containing more than only one atom.

126
Q

Polymer

A

A large molecule formed from many thousands of repeat units of smaller molecules known as monomers

127
Q

Position of equilibrium

A

The relative quantities of reactants and products, indicating the extent of a reversible reaction at equilibrium

128
Q

Primary

A

On a carbon atom at the end of a chain

129
Q

Primary alcohol

A

An alcohol in which the -OH group is attached to a carbon atom that is attached to two or three hydrogen atoms

130
Q

Principle quantum number n

A

A number representing the relative overall energy of each orbital, which increases with distance from the nucleus. The sets of orbitals with the same n-value are referred to as electron shells or energy levels

131
Q

Propagation

A

the steps that continue a free radical reaction in which a radical reacts with a reactant molecule to form a new molecule and another radical, causing a chain reaction

132
Q

Proton number

A

The number of protons in the nucleus of an atom; also known as atomic number

133
Q

Radical

A

A species with an unpaired electron

134
Q

Rate of reaction

A

The change in concentration of a reactant or a product in a given time

135
Q

Reaction mechanism

A

The sequence of bond breaking and bond-forming steps that shows the path taken by electrons during a reaction

136
Q

Redox reaction

A

A reaction involving reduction and oxidation

137
Q

Reducing agent

A

A reagent that reduces (adds electron to) another species

138
Q

Reduction

A

Gain of electrons or a decrease in oxidation number

139
Q

Reflux

A

The continual boiling and condensing of a reaction mixture back to the original container to ensure that the reaction takes place without the contents of the flask boiling dry

140
Q

Relative atomic mass Ar

A

The weighted mean mass of an atom of an element compared with one-twelfth of the mass of an atom of carbon-12

141
Q

Relative formula mass

A

The weighted mean mass of the formula unit of a compound compared with one-twelfth of the mass of an atom of carbon-12

142
Q

Relative isotopic mass

A

The mass of an isotope compared with one-twelfth of the mass of an atom of carbon-12

143
Q

Relative molecular mass Mr

A

The weighted mean mass of a molecule of a compound compared with one-twelfth of the mass of an atom of carbon-12

144
Q

Reversible reaction

A

A reaction that takes place in both forward and reverse directions

145
Q

σ-bond

A

Sigma bond, a bond formed by the overlap of one orbital from each bonding atom, consisting of two electrons and with the electron density centred around a line directly between the nuclei of the two atoms

146
Q

Salt

A

The product of a reaction in which the H+ ions from the acid are replaced by metal or ammonium ions

147
Q

Saturated

A

Containing single bonds only

148
Q

Saturated hydrocarbon

A

A hydrocarbon with single bonds only

149
Q

Second ionisation energy

A

The energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element to form one mole of gaseous 2+ ions

150
Q

Secondary

A

On a carbon atom to which two carbon chains are attached

151
Q

Shell (electron shell)

A

A group of atomic orbitals with the same principal quantum number n. Also known as a main energy level

152
Q

Shielding effect

A

The repulsion between electrons in different inner shells. Shielding reduces the net attractive force between the positive nucleus on the outer shell electrons

153
Q

Simple molecular lattice

A

A three-dimensional structure of molecules, bonded together by weak intermolecular forces

154
Q

Skeletal formula

A

A simplified organic formula, with hydrogen atoms removed from alkyl chains, leaving just a carbon skeleton and associated functional groups

155
Q

Specific heat capacity, c

A

The energy required to raise the temperature of 1g of a substance by 1K

156
Q

Standard enthalpy change of combustion ΔcH°

A

The enthalpy change that occurs when one mole of a substance reacts completely with oxygen under standard conditions, with all reactants and products in their standard states

157
Q

Standard enthalpy change of formation ΔfH°

A

The enthalpy change that occurs when one mole of a compound is formed from its elements under standard conditions, with all reactants and products in their standard states

158
Q

Standard enthalpy change of neutralisation ΔneutH°

A

The enthalpy change that accompanies the reaction of an acid by a base to form one mole of H2O(l), under standard conditions, with all reactants and products in their standard states.

159
Q

Standard enthalpy change of reaction ΔrH°

A

The enthalpy change that accompanies a reaction in the molar quantities shown in a chemical equation under standard conditions, with all reactants and products in their standard states

160
Q

Standard solution

A

A solution of known concentration

161
Q

Standard state

A

The physical state of a substance under standard conditions of 100kPa and a stated temperature (usually 298K)

162
Q

Stereoisomers

A

Compounds with the same structural formula but with a different arrangement of the atoms in space

163
Q

Stoichiometry

A

The ratio of the amount, in moles, of each substance in a chemical reaction

164
Q

Strong acid

A

An acid that dissociates completely in solution

165
Q

Structural formula

A

A formula showing the minimal detail for the arrangement of atoms in a molecule

166
Q

Structural isomers

A

Compounds with the same molecular formula but different structural formulae

167
Q

Sub-shell

A

A group of orbitals of the same type within a shell

168
Q

Substitution reaction

A

A reaction in which one atom or group of atoms ins replaced by another atom or group of atoms

169
Q

Surroundings

A

Everything that is not the chemical system

170
Q

System

A

Everything - the atoms, molecules, or ions - making up the chemical compounds being studied

171
Q

Termination

A

The step at the end of a radical substitution when two radicals combine to form a molecule

172
Q

Tertiary

A

On a carbon atom to which three carbon chains are attached

173
Q

Tertiary alcohol

A

An alcohol in which the -OH group is attached to a carbon atom that is attached to no hydrogen atoms

174
Q

Theoretical yield

A

The yield resulting from complete conversion of reactants into products

175
Q

Unsaturated

A

Containing a multiple carbon-to-carbon bond

176
Q

Water of crystallisation

A

Water molecules that are bonded into a crystalline structure of a compound

177
Q

Weak acid

A

An acid that dissocates only partially in solution

A Level Chemistry (OCR) - Memorise (3 decks)

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